Question

In: Chemistry

a) Refrigerators and freezers remove heat from food by evaporating volatile liquids such as CF4 and...

a) Refrigerators and freezers remove heat from food by evaporating volatile liquids such as CF4 and then recompressing the vapor back into a liquid. Calculate what mass of water at 0.0 deg C can be converted into ice at 0.0 deg C when 1.00 kg of CF4 evaporates. (delta Hvap = 136 kJ/kg for CF4)

b) Water in a leather flask or a porous clay pot can be cooled in hot climates by evaporating water from the surface of the container. Calculate what mass of water can be cooled from 35 deg C to 20 deg C via the evaporation of 60 g of water

Solutions

Expert Solution

Ans. #A. Amount of heat absorbed during vaporization of 1 kg CF4 = dHvap x Mass of CF4

                                                = (136 kJ/ kg) x 1.0 kg

                                                = 136 kJ

# The heat is absorbed from liquid water by CF4.

So, total heat lost from water = -136 kJ. The –ve sign indicates that heat is lost from water.

# Now, heat lost by water is given by-

q = m C                                 - equation 1

Where,

q = heat gained

m = mass

C = enthalpy of fusion of ice

Or,

            136 kJ = m x (333.55 kJ/ kg)

            Or, m = 136 kJ / (333.55 kJ/ mol)

            Hence, m = 0.407734 kg

Hence, required mass of water converted into ice at 0.00C = 0.407734 kg

                                                = 407.734 g

#B. Total heat absorbed during valorization of 60.0 g water = dHvap x mass of water

                                    = (2257.0 J / g) x 60.0 g

                                    = 135420 J

# The heat absorbed during vaporization is extracted from liquid water to cool it.

So,

Amount of heat lost by water during cooling = 135420 J

Now,

Heat lost by water given by-

q = m s dT                            - equation 1

Where,

q = heat lost

m = mass

s = specific heat

dT = Final temperature – Initial temperature

Or,

            135420 J = m x (4.184 J g-10C-1) x (35.0 – 20.0)0C

            Or, 135420 J = m x 62.76 J g-1

                Or, m = 135420 J / (62.76 J g-1)

            Hence, m = 2157.74 g

Hence, required mass of water = 2157.74 g = 2.158 kg


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